Transition And Polyatomic Ions 2008

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Transition And Polyatomic Ions 2008

  1. 1. Transition Metals & Polyatomic Ions
  2. 2. Goal 1 Name ionic compounds that contain transition metals
  3. 3. <ul><li>Transition Metals </li></ul><ul><ul><li>Total charge on compound = 0 </li></ul></ul><ul><ul><li>Electron loss can vary </li></ul></ul><ul><ul><li>Roman numerals </li></ul></ul><ul><ul><ul><li>Indicate charge </li></ul></ul></ul>
  4. 4. <ul><li>Step 1: Determine total charge on nonmetal </li></ul>MnO O = 2- Fe 2 S 3 S 3 = 6-
  5. 5. <ul><li>Step 2: Determine needed charge on transition metal to create an equal opposite charge (multiply by subscript) </li></ul>MnO Mn = 2+ O = 2- Fe 2 S 3 Fe = 3+ S 3 = 6-
  6. 6. <ul><li>Step 3: Use charge on transition metal to determine your roman numeral </li></ul>MnO Mn = 2+ O = 2- manganese(II) oxide Fe 2 S 3 Fe = 3+ S 3 = 6- iron(III) sulfide
  7. 7. <ul><li>Try it backwards! </li></ul><ul><li>Chemical formula from a name </li></ul>Tin(II) oxide
  8. 8. <ul><li>Step 1: Determine charge on transition metal </li></ul>Tin(II) oxide Sn = 2+
  9. 9. <ul><li>Step 2: Determine charge on nonmetal ion </li></ul><ul><li>(use periodic table) </li></ul>Tin(II) oxide Sn = 2+ O = 2-
  10. 10. <ul><li>Step 3: Determine how many of each needed to equal 0 charge (CC&R) </li></ul>Tin(II) oxide Sn = 2+ O = 2- SnO
  11. 11. <ul><li>Try it… </li></ul><ul><li>Iron(III) fluoride </li></ul>
  12. 12. <ul><li>Were you correct? </li></ul><ul><li>Iron(III) fluoride </li></ul><ul><li>FeFl 3 </li></ul>
  13. 13. <ul><li>Try again (this time backwards) </li></ul><ul><li>TiN </li></ul>
  14. 14. <ul><li>Were you correct? </li></ul><ul><li>TiN </li></ul><ul><li>titanium(III) nitride </li></ul>
  15. 15. <ul><li>And again… </li></ul><ul><li>PbO 2 </li></ul>
  16. 16. <ul><li>Were you correct? </li></ul><ul><li>PbO 2 </li></ul><ul><li>lead(IV) oxide </li></ul>
  17. 17. Goal 2 Name ionic compounds using polyatomic ions
  18. 18. <ul><li>Polyatomic ions </li></ul><ul><ul><li>Covalently bonded elements with a charge </li></ul></ul><ul><ul><li>May be indicated by parentheses </li></ul></ul>(OH - ) (OH - ) 2
  19. 19. <ul><ul><li>Use the same as a single ion </li></ul></ul><ul><ul><li>Information found on back of periodic table </li></ul></ul>Hydroxide ion
  20. 20. <ul><li>Step 1: recognize use of polyatomic ion </li></ul><ul><ul><li>Name ends in “- ate ” or “- ite ” </li></ul></ul><ul><ul><li>Name that is not an element… cyanide </li></ul></ul><ul><ul><li>Parentheses used in chemical formula </li></ul></ul><ul><ul><li>Or… check anyways </li></ul></ul>Sodium sulf ate Na 2 (SO 4 )
  21. 21. <ul><li>Step 2: use back of your periodic table to determine charge on the polyatomic ion </li></ul>Sodium sulfate 2-
  22. 22. <ul><li>Step 3: determine how many metal ions needed to make a 0 charge (criss-cross) </li></ul>Sodium 1+ 2 sulfate 2- Na 2 (SO 4 )
  23. 23. <ul><li>Try it…. </li></ul><ul><li>Calcium chlorate </li></ul>
  24. 24. <ul><li>Try it…. </li></ul><ul><li>Calcium chlor ate </li></ul>
  25. 25. <ul><li>Try it…. </li></ul><ul><li>Calcium chlorate 1- </li></ul>
  26. 26. <ul><li>Try it…. </li></ul><ul><li>Calcium 2+ chlorate 1- 2 </li></ul><ul><li>Ca(ClO 3 ) 2 </li></ul>CC&R stays OUTSIDE of polyatomic parentheses
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